Question

For the decomposition of barium carbonate, consider the following thermodynamic data:

ΔrH∘ΔrH∘	271.5kJ mol−1
ΔrS∘ΔrS∘	173.8J K−1 mol−1

A: Calculate the temperature in kelvins above which this reaction is spontaneous.

Answer:1562K

B: Calculate the equilibrium constant for the following reaction at room temperature, 25 ∘C:

BaCO3(s)→BaO(s)+CO2(g)

Answer: 2.73*10^-39

C: When adjusted for any changes in ΔrH and ΔrS with temperature, ΔrG∘(600K)=167kJ mol−1. Calculate the equilibrium constant at 600 K .

Answer 1

THE SOLUTION FOR THIS QUESTION IS AS FOLLOWS

AGATAS Gevon A Hy 271.5 kulmol .. AS, 113.2 Kamalk loro best spontaneous <0,30 Here is assump Hemat T entot at which oc=0 = 2115 - T x 13.2 a loro 2115x115 T= 1562-14K 30 25 6 = A4 = AH - TAS 2-1:3- 298 x 1732 AG-811.5 - 5.7929 AG 19. 1076 kamole AG - RTlnk - 14.7076X1o 3 - 8:3/4 X24 -88 6785Ink . 38.505 Look K-2.13 X 10 - 39 e-COPY

AG= - RTlnk. A. - 2.303 RT Logk 167 x103 -2.303 x Geox 8.3 4 Logk = -167x103 07.3.3.x 600 x 8-314 Look - - 14.53 K= 2.95 x 10-15